Each group of elements having the same number of valence electrons. , Electrons and Sublevels  Electron Configurations and the Periodic Table  Writing Electron Configurations  Box and Arrow Configurations using Pauli Exclusion Principle and Hund's Rule   Quantum Numbers, Electron Configurations and the Periodic Table, Electron configurations and the periodic table. = 7 + 10 = 17) Question 11. Likewise, the outer shell moves further from the nucleus. (adsbygoogle = window.adsbygoogle || []).push({}); © Copyright 2021 W3spoint.com. Then its period number is 3 as it has three electrons shells. The reaction is faster. Table 2: Reaction of halogens with iron wool. (AI 2016) Answer: Atomic number of X = Mass number of X – No of neutrons = 35 – 18 = 17 Therefore Electronic configuration of X = 2, 8, 7 Group number =17 Physical and Chemical Properties of Aldehydes and Ketones, Oxidation states of d and f Block Elements, Electronic Configuration of Group 14 Elements, Physical and chemical properties of Group 16 elements. Which group of elements has the valence configuration of {eq}ns^2np^2 {/eq}? There is more attraction which makes it easier to gain an extra electron. This results in the valence shell being shielded by more inner electron shells. Atomic number of given element = 17 ∴ Electronic configuration of given element = 2, 8, 7 (a) Valency = 1 Since this element requires one electron to complete its octet (outermost shell). Halogens gain an electron in reactions to form negative ions with a -1 charge and they are 1 electron less than a full octet. The electronic configuration of any element determines its physical state and reactivity with other elements. They use these electrons in the bond formation in order to obtain octet configuration. As we learned earlier, each neutral atom has a number of electrons equal to its number of protons. (ii) A common feature of the electronic configuration of the elements at the end of Period 2 and Period 3 is that the atoms have 8 electrons in their outermost shell. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. Hence they are kept in group VII-A (17) of a periodic table, before inert gases. The general electronic configuration of the d-block elements is (n − 1)d 1–10 ns 0–2.Here "(noble gas)" is the configuration of the last noble gas preceding the atom in question, and n is the highest principal quantum number of an occupied orbital in that atom. The element misses out on the octet configuration by one electron. The general electronic configuration of group 17 is: ns2np5. google_ad_height = 60; Caesium (Cs) 7. The atoms of each element gain more shells and increase in size going down the group. The penultimate shell of carbon contains the s 2 electrons, silicon has s 2 p 6 electrons and germanium contains the s 2 p 6 d 10 electrons and is unsaturated. The elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) are called the halogens. The same goes for bromine (4s 2 4p 5 ), iodine (4s 2 4p 5 ), and astatine (5s 2 5p 5 ).Thus it is ironic that they are neighbors to the Group 8 noble gases, the least reactive among the elements. For example, all the elements in group 13, beginning with boron, end with “p1”. Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At) in the periodic table belong to group-17, or VIIA with the general electronic configuration of valence electron ns 2 np 5, where n = 2 to 6. The manufacturing of these compounds can only be performed under extreme conditions of high temperature and pressure. The elements are Hydrogen and Helium with electronic configuration 1s 1 and 1s 2 This marks the complete filling of K shell. Properties of Halogens: Monovalency of Halogens: All halogen have shell electronic configuration is … They share unpaired electrons to form covalent bonds as well. The s-, p- and d-block elements of the periodic table are arranged into these columns or groups. The compounds of the s-block elements, with the exception of those of beryllium are predominantly ionic. p-Block Elements The p-Block Elements comprise those belonging to groups 13 to 18 and together with the s-block elements are called the Representative Elements or Main Group Elements. Therefore, these are very reactive non-metals. Write the period number, c. What will be the chemical formula of the compound formed if the element X reacts with element Y of the third period which contains one electron in the p subshell? The general rule is that the element's electron configuration ends in d and whatever place they are in. All Group 17 (group VIIA or halogen) elements have 7 valence electrons (7 electrons in the valence shell or highest energy level ). It is the first column of the s block of the periodic table. Thus, these elements look out to either lose one electron and form a covalent bond or gain one electron and form an ionic bond. The “f  block” elements are those at the bottom of the periodic table that we call the lanthanide and actinide groups. For example, the s sublevel can only hold two electrons, so the 1s is filled at helium (1s 2).The p sublevel can hold six electrons, the d sublevel can hold 10 electrons, and the f sublevel can hold 14 electrons. Here is a summary of the types of orbitals and how many electrons each can contain: So based on what we know about the quantum numbers and using the char… (b) This element is a non-metal as it gains one electron to complete its outermost shell and elements which gain electrons … Write atomic number and electronic configuration of ‘X’. The transition elements are called “d block” elements and always end with 1 or more “d electrons”. Although astatine is radioactive and only has short-lived isotopes, it behaves similar to iodine … The first example occurs in the case of the lanthanoids (elements having atomic numbers between 57 and 71).The lanthanoids have the general electron configuration [Kr]4d 10 4f i 5s 2 5p 6 5d 0 or 1 6s 2. where i is a number between 0 and 14. They can easily obtain a full octet by gaining one electron. Lithium (Li) 3. Actual configurations have not been verified. Atomic radius increases down Group 17 from top to bottom. The halogens all have the general electron configuration n s 2n p 5, giving them seven valence electrons. The third major category of elements arises when the distinguishing electron occupies an f subshell. There are 118 elements … Forming compounds. The element X in group 17 has 3 shells. b. Therefore, astatine is a metalloid which prefers sharing or losing electrons to become an unstable and radioactive compound. And so it goes. To form a compound in a chemical reaction, electrons must be exchanged. They can easily obtain a full octet by gaining one electron. The reaction is slow. Write the subshell electronic configuration of the element. Fluorides of Krypton and compounds of xenon, such as Oxides, fluorides, and oxyfluorides, are well known. Hydrogen (H) 2. The general electronic configuration is ns2np5 and the last electron occupies p orbital. The Same group elements have similar properties and reactivity. Scandium would end in 3d1, titanium in 3d2, etc. Login, Best Place for Technologies and Academics Tutorial, p-Block Elements: Group 17 (Electronic configuration). (∵ Group no. Also write group number, period number and valency of ‘X’. Very few scientists handle fluorine because it is so dangerous. Table 1: Electronic configuration of group 17 elements. The form of the periodic table is closely related to the electron configuration of the atoms of the elements. Example: If the electronic configuration of an element is 2, 8, 7. These elements are a part of the p block. Three shells are K, L, M. Therefore fluorine is the most reactive and it produces stable ionic salts and covalent compounds due to highest electronegativity. An element ‘X’ has mass number 35 and number of neutrons 18. For example, the all of the elements in group 3 beginning with scandium, all end in “d1”. The members of this group 1 are as follows: 1. They are one electron short of having full outer s … There are seven electrons in the outermost shell. They are one electron short of having full outer s … google_ad_client = "pub-0644478549845373"; The rows in the periodic table show increasing energy levels and the levels rise as one moves up the list of halogens. google_ad_width = 468; All of the elements in group 16, beginning with oxygen, end with “p4”. Rhubidium (Rh) 6. (iii) If an element is in Group 17, it is likely to be non-metallic in character, while with one electron in its outermost energy level (shell), then it is likely to be metallic. Properties and Trends in Element 14 1) Covalent Radius. Group 1 elements are chemical elements having an unpaired electron in the outermost s orbital. The halogens all have the general electron configuration ns2np5, giving them seven valence electrons. For instance, hydrogen exists as a gas, while other ele… Electron configurations are the summary of where the electrons are around a nucleus. Fluorine, on row 2, has a valence-shell configuration of 2s 2 2p 5; while that of chlorine is 3s 2 3p 5. These elements require one electron to finish their octet. All rights reserved. The electronic configurations of the elements in group 1: The atoms of all group 1 elements have similar chemical properties and reactions because they all have one electron in their outer shell. Potassium (K) 5. For example, all the elements of group 2 have an electron configuration of [E] ns 2 (where [E] is an inert gas configuration), and have notable similarities in their chemical properties. Answer: a. The alkali metal electron configurations (group 1) always end with “s1” and the alkaline earth metals (group 2) always end with “s2”. Electronegativity decreases down group 17 from top to bottom. 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